MCQs for Chemistry Class 11 with Answers Chapter 4 Chemical Bonding and Molecular Structure
Students of class 11 Chemistry should refer to MCQ Questions Class 11 Chemistry Chemical Bonding and Molecular Structure with answers provided here which is an important chapter in Class 11 Chemistry NCERT textbook. These MCQ for Class 11 Chemistry with Answers have been prepared based on the latest CBSE and NCERT syllabus and examination guidelines for Class 11 Chemistry. The following MCQs can help you to practice and get better marks in the upcoming class 11 Chemistry examination
Chapter 4 Chemical Bonding and Molecular Structure MCQ with Answers Class 11 Chemistry
MCQ Questions Class 11 Chemistry Chemical Bonding and Molecular Structure provided below have been prepared by expert teachers of grade 11. These objective questions with solutions are expected to come in the upcoming Standard 11 examinations. Learn the below provided MCQ questions to get better marks in examinations.
Question. Among the following, electron deficient molecule is
Question. Sodium chloride is soluble in water but not in benzene because
(a) ΔHHydration < ΔHLattice energy in water
ΔHHydration > ΔHLattice energy in benzene
(b) ΔHHydration > ΔHLattice energy in water
ΔHHydration < ΔHLattice energy in benzene
(c) ΔHHydration = ΔHLattice energy in water
ΔHHydration < ΔHLattice energy in benzene
(d) ΔHHydration < ΔHLattice energy in water
ΔHHydration = ΔHLattice energy in benzene
Question. Which of the following compounds contain(s) no covalent bond(s)?
KCl, PH3,O2, B2H6, H2SO4
(a) KCl2, BH6, PH3
(b) KCl, H2 SO4
(d) KCl, B2 H6
Question. The % ionic character in Cs—Cl bond present in CsCl molecule will be, if the electronegativity values or Cs and Cl are 0.8 and 3.0 respectively
Question. Which one of the following molecule is polar?
Question. Which of the following pairs has zero dipole moment?
(a) CH2 Cl2 and NF3
(b) SiF4 and BF3
(c) PCl and ClF 3
(d) BF3 and NF 3
Question. Bond distance in HF is 9.17 10 m × −11 . Dipole moment of HF is 6.104 10 cm × −30 . The per cent ionic character in HF will be (electron charge = 1.60 × 10− C 19 )
Question. Among the following the maximum covalent character is shown by the compound
Question. The correct statement for the molecule,CsI3 is
(a) it is a covalent molecule
(b) it contains Cs+ and I3−
(c) It contains Cs3+ and I− ions
(d) it contains Cs+ ,I− and lattice I2 molecule
Question. Which of the following compounds has the smallest bond angle in its molecule?
Question. Which of the following statement(s) is/are true?
(a) HF is less polar than HBr
(b) Absolutely pure water does not contain any ions
(c) Chemical bond formation takes place when forces of attraction overcome the forces of repulsion
(d) In covalency, transference of electrons take place
Question. Which of the following molecules/ions does not contain unpaired electrons ?
Question. Which of the following species has a bond order other than 3?
Question. The sequence that correctly describes the relative bond strength pertaining to oxygen molecule and its cation or anion is
(a) O22- ,> O2– > O2 > O2+
(b) O2,> O2+ > O2–> O22-
(c) O2+ ,> O2 > O22-> O2–
(d) O2+ ,> O2 > O–2 > O22-
Question. The bond order of o; is the same as in
Question. Molecular orbital theory was given by
Question. What is the geometry of nitrogen atom inNH3 , N(CH3 )3 and N[Si(CH3 )3 ]3 molecules?
I. Trigonal planar
II. Trigonal pyramidal
III. Square planar
Choose the correct option.
(a) II, II and I
(b) III, III and I
(c) I, II and III
(d) I, III and II
Question. O2 molecule is paramagnetic due to the presence of
(a) two unpaired electrons in anti-bonding MO
(b) one unpaired electron in anti-bonding MO
(c) two unpaired electrons in bonding MO
(d) one unpaired electron in bonding MO
Question. The BCl3 is a planar molecule whereasNCl3 is pyramidal because
(a) B—Cl bond is more polar than N—Cl bond
(b) N—Cl bond is more covalent that B—Cl bond
(c) nitrogen atom is smaller than boron atom
(d) BCl3 has no lone pair electrons butNCl3 has one lone pair of electrons
Question. H2O is dipolar whereas BeF2 is not. It is because
(a) the electronegativity of F is greater than that of O
(b) H2O involves hydrogen bonding whereas BeF2 is angular discrete molecule
(c) H2O is linear and BeF2 is angular
(d) H2O is angular and BeF2 is linear
Question. In terms of polar character, which one of the following order is correct?
(a) NH3 < H2O < HF < H2S
(b) H2S < NH3 < HO < HF
(c) H2O < NH3 < HS < HF
(d) HF < H2O < NH3 < H2S
Question. What will be the lattice enthalpy of CaCl2, if the enthalpy of
(i) sublimation energy of Ca is 121 kJmol−1
(ii) dissociation energy of Cl2 to Cl is 242.8 kJmol−1
(iii) ionisation energy Ca to Ca2+ is 2422 kJmol−1
(iv) electron gain enthalpy for Cl to Cl– is −355 kJ mol−1
(v) ΔfH overall is −795 kJ mol−1
(a) −3225.8 kJ mol−1
(b) −980.8 kJ mol−1
(c) −2870.8 kJ mol−1
(d) −2628 kJ mol−1
Question. Select the correct statement(s).
(a) Both lattice energy and hydration energy decrease with the increase in ionic size
(b) Lattice energy can be calculated using Born-Haber cycle
(c) If the anion is larger than the cation, the lattice energy will remain almost constant within a particular group
(d) All of the above statements are correct
Question. The bond dissociation energy of B—F in BF3 is 646 kJ mol−1, whereas that of C—F in CF4 is 515 kJ mol−1. The correct reason for higher B—F bond dissociation energy as compared to that of C—F bond is
(a)smaller size of B-atom as compared to that of C-atom
(b) stronger s bond between B and F in BF3 as compared to that between C and F isCF4
(c) significant pp-pp interaction between B and F in BF3 whereas there is no possibility of such interaction between C and F in CF4
(d) lower degree of pp-pp interaction betwen B and F in BF3 than that between C and F inCF4
Question. If H—X bond length is 2A ° and H−X bond has dipole moment 512 × 10−30 . cm, the percentage of ionic characters in the molecule will be
Question. The geometrical shapes of XeF5+ , XeF6 and XeF82− respectively are
(a) trigonal bipyramidal, octahedral and square planar
(b) square pyramidal, distorted octahedral and square antiprismatic
(c) planar pentagonal, octahedral and square antiprismatic
(d) square pyramidal, distorted octahedral and octahedral
Question. The number of antibonding electron pairs in O2-2 molecular ion on the basis of molecular orbital theory is (Atomic number ofO is 8.)
Question. Which of the following is paramagnetic with bond order 0.5?
Question. N2 accept electron and convert into N;, where this electron goes?
(a) Antibonding n-molecular orbital
(b) Bonding n-molecular orbital
(c) σ-bonding molecular oribital
(d) σ-antibonding molecular orbital
Question. The formation of energy bonds in solids are in accordance with
(a) Heisenberg’s uncertainty principle
(b) Bohr’s theory
(c) Ohm’s law
(d) Rutherford’s atomic model
Question. Which of the following is isoelectronic with CO2?
Question. Suppose the observed value of dipole moment of H2O molecule is 1.83 D. What will be the H—O—H bond angle in H2O molecule? (Given bond moment of O—H bond is 1.5 D.)
(a) 104° 20¢¢
Question. Which one of the following molecules is/are expected to exhibited diamagnetic behaviour?
Question. Which of the following statement(s) is/are correct?
(a) In the formation of dioxygen from oxygen atoms 10 molecular orbitals will be formed.
(b) All the molecular orbitals in the dioxygen will be completely filled
(c) Total number of bonding molecular orbitals will not be same as total number of anti-bonding orbitals n dioxygen
(d) Number of filled bonding orbitals will be same as number of filled anti-bonding orbitals
Question. In accordance to molecular theory,
(a) O2+ is diamagnetic and bond order is more thanO2
(b) O2+ is diamagnetic and bond order is less thanO2
(c) O2+ is paramagnetic and bond order is more thanO2
(d) O2+ is paramagnetic and bond order is less thanO2
Question. Which of the following pairs of molecules/ions are not likely to exist?
(a) H2+, He22−
(b) H2−, He−22
(c) H22+ , He2
(d) H2− , He2+2
Question. Ortho-nitrophenol is less soluble in water than p-andm-nitrophenols because
(a) o -nitrophenol is more steam volatile than those of m- and p -isomers
(b) o -nitrophenol shows intramolecular H-bonding
(c) o -nitrophenol shows intermolecular H-bonding
(d) melting point of o -nitrophenol is lower than those of m- and p-isomers
Question. Arrange the following molecules in the increasing order of bond angle.
H2O H2S H2Se H2Te I II III IV
(a) I < II < III < IV
(b) IV < III < II < I
(c) I < III <II < IV
(d) IV < II < III < I
Question. Consider the following iodides, PI3 102 ¾ °, AsI3 100.2, ¾ SbI3 99 ¾ ° The bond angle is maximum in P 3 I which is
(a) due to small size of phosphorus
(b) due to more bp-bp repulsion in P 3 I
(c) due to less electronegativity of phosphorus
(d) None of the above
Question. Bond energy of H—H, F—F and H—F bonds are 104, 38 and 135 kcal mol−1 respectively. The resonance energy in the H—F molecule will be
(a) 142 kcal mol−1
(b) 66 kcal mol−1
(c) 72.14 kcal mol−1
(d) 79.26 kcal mol−1
Question. The species in which the N-atom is in a state of sp- hybridisation is
Question. The d-orbital involved in sp3 d -hybridisation is
(d) dx2 −y2
Question. The states of hybridisation of boron and oxygen atoms in boric acid (H3BO3 ) are respectively
(a) sp2 and sp3
(b) sp2 and sp3
(c) sp3 and sp2
(d) sp3 and sp3
Question. Isostructural species are those which have the same shape and hybridisation. Among the given pecies identify the isostructural pairs.
(a) NF3 and BF 3
(b) BF4− and NH4+
(c) BCl3 and BrCl3
(d) NH3 and NO–3
Question. In which of the following pairs the two species are not isostructural?
(a) CO32− and NO3−
(b) PCl4+ and SiCl4
(c) PF5 and BrF5
(d) AlF63− and SF6
Question. Total number of lone pair of electron in I3− ion is
Question. In XeF2, XeF4 and XeF6, the number of lone pairs of Xe respectively are
(a) 2, 3, 1
(b) 1, 2, 3
(c) 4, 1, 2
(d) 3, 2, 1
Question. The structure of IF7 is
(a) square pyramidal
(b) trigonal bipyramidal
(d) pentagonal bipyramidal
Question. Which has trigonal bipyramidal shape?
(c) XeO3 F2
Question. The shape of IF6− is
(a) trigonally distorted octahedron
(d) square antiprism
Question. The molecular shapes of SF4 , CF4 and XeF4 are
(a) different with 1, 0 and 2 lone pairs of electrons on the central atoms, respectively
(b) different with 0, 1 and 2 lone pairs of electrons on the central atoms, respectively
(c) the same with 1, 1 and 1 lone pairs of electrons on the central atoms, respectively
(d) the same with 2, 0 and 1 lone pairs of electrons on the central atoms, respectively
Question. The structure of which of the following chloro species can be explained on the basis of dsp2- ybridisation ?
Question. XeO4 molecule is tetrahedral having
(a) two pΠ − dΠ bonds
(b) one pΠ − dΠ bond
(c) four pΠ − dΠ bonds
(d) three pΠ − dΠbonds
Question.Which of the following species is not paramagnetic?
We hope the above multiple choice questions for Class 11 Chemistry for Chapter 4 Chemical Bonding and Molecular Structure provided above with answers based on the latest syllabus and examination guidelines issued by CBSE, NCERT and KVS are really useful for you. Chemical Bonding and Molecular Structure is an important chapter in Class 11 as it provides very strong understanding about this topic. Students should go through the answers provided for the MCQs after they have themselves solved the questions. All MCQs have been provided with four options for the students to solve. These questions are really useful for benefit of class 11 students. Please go through these and let us know if you have any feedback in the comments section.